This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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Here are the solutions to the questions: SECTION - I Q#2: Give Short Answers to the following questions. (Any EIGHT) 1. Why diamond is a non-conductor while graphite is conductor? In diamond*, each carbon atom is sp^3 hybridized and forms four strong sigma bonds with other carbon atoms. All valence electrons are localized in these bonds, so there are no free electrons to conduct electricity. In graphite*, each carbon atom is sp^2 hybridized and forms three sigma bonds. The remaining unhybridized p-orbitals overlap to form a delocalized pi electron cloud above and below the planes. These delocalized electrons are free to move, making graphite a good electrical